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CaSO4 + AlBr3 = Al2(SO4)3 + CaBr2

Input interpretation

CaSO_4 calcium sulfate + AlBr_3 aluminum tribromide ⟶ Al_2(SO_4)_3 aluminum sulfate + CaBr_2 calcium bromide
CaSO_4 calcium sulfate + AlBr_3 aluminum tribromide ⟶ Al_2(SO_4)_3 aluminum sulfate + CaBr_2 calcium bromide

Balanced equation

Balance the chemical equation algebraically: CaSO_4 + AlBr_3 ⟶ Al_2(SO_4)_3 + CaBr_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CaSO_4 + c_2 AlBr_3 ⟶ c_3 Al_2(SO_4)_3 + c_4 CaBr_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Ca, O, S, Al and Br: Ca: | c_1 = c_4 O: | 4 c_1 = 12 c_3 S: | c_1 = 3 c_3 Al: | c_2 = 2 c_3 Br: | 3 c_2 = 2 c_4 Since the coefficients are relative quantities and underdetermined, choose a coefficient to set arbitrarily. To keep the coefficients small, the arbitrary value is ordinarily one. For instance, set c_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 2 c_3 = 1 c_4 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 CaSO_4 + 2 AlBr_3 ⟶ Al_2(SO_4)_3 + 3 CaBr_2
Balance the chemical equation algebraically: CaSO_4 + AlBr_3 ⟶ Al_2(SO_4)_3 + CaBr_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CaSO_4 + c_2 AlBr_3 ⟶ c_3 Al_2(SO_4)_3 + c_4 CaBr_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Ca, O, S, Al and Br: Ca: | c_1 = c_4 O: | 4 c_1 = 12 c_3 S: | c_1 = 3 c_3 Al: | c_2 = 2 c_3 Br: | 3 c_2 = 2 c_4 Since the coefficients are relative quantities and underdetermined, choose a coefficient to set arbitrarily. To keep the coefficients small, the arbitrary value is ordinarily one. For instance, set c_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 2 c_3 = 1 c_4 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 CaSO_4 + 2 AlBr_3 ⟶ Al_2(SO_4)_3 + 3 CaBr_2

Structures

+ ⟶ +
+ ⟶ +

Names

calcium sulfate + aluminum tribromide ⟶ aluminum sulfate + calcium bromide
calcium sulfate + aluminum tribromide ⟶ aluminum sulfate + calcium bromide

Equilibrium constant

Construct the equilibrium constant, K, expression for: CaSO_4 + AlBr_3 ⟶ Al_2(SO_4)_3 + CaBr_2 Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the activity expression for each chemical species. • Use the activity expressions to build the equilibrium constant expression. Write the balanced chemical equation: 3 CaSO_4 + 2 AlBr_3 ⟶ Al_2(SO_4)_3 + 3 CaBr_2 Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i CaSO_4 | 3 | -3 AlBr_3 | 2 | -2 Al_2(SO_4)_3 | 1 | 1 CaBr_2 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression CaSO_4 | 3 | -3 | ([CaSO4])^(-3) AlBr_3 | 2 | -2 | ([AlBr3])^(-2) Al_2(SO_4)_3 | 1 | 1 | [Al2(SO4)3] CaBr_2 | 3 | 3 | ([CaBr2])^3 The equilibrium constant symbol in the concentration basis is: K_c Mulitply the activity expressions to arrive at the K_c expression: Answer: | | K_c = ([CaSO4])^(-3) ([AlBr3])^(-2) [Al2(SO4)3] ([CaBr2])^3 = ([Al2(SO4)3] ([CaBr2])^3)/(([CaSO4])^3 ([AlBr3])^2)
Construct the equilibrium constant, K, expression for: CaSO_4 + AlBr_3 ⟶ Al_2(SO_4)_3 + CaBr_2 Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the activity expression for each chemical species. • Use the activity expressions to build the equilibrium constant expression. Write the balanced chemical equation: 3 CaSO_4 + 2 AlBr_3 ⟶ Al_2(SO_4)_3 + 3 CaBr_2 Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i CaSO_4 | 3 | -3 AlBr_3 | 2 | -2 Al_2(SO_4)_3 | 1 | 1 CaBr_2 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression CaSO_4 | 3 | -3 | ([CaSO4])^(-3) AlBr_3 | 2 | -2 | ([AlBr3])^(-2) Al_2(SO_4)_3 | 1 | 1 | [Al2(SO4)3] CaBr_2 | 3 | 3 | ([CaBr2])^3 The equilibrium constant symbol in the concentration basis is: K_c Mulitply the activity expressions to arrive at the K_c expression: Answer: | | K_c = ([CaSO4])^(-3) ([AlBr3])^(-2) [Al2(SO4)3] ([CaBr2])^3 = ([Al2(SO4)3] ([CaBr2])^3)/(([CaSO4])^3 ([AlBr3])^2)

Rate of reaction

Construct the rate of reaction expression for: CaSO_4 + AlBr_3 ⟶ Al_2(SO_4)_3 + CaBr_2 Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the rate term for each chemical species. • Write the rate of reaction expression. Write the balanced chemical equation: 3 CaSO_4 + 2 AlBr_3 ⟶ Al_2(SO_4)_3 + 3 CaBr_2 Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i CaSO_4 | 3 | -3 AlBr_3 | 2 | -2 Al_2(SO_4)_3 | 1 | 1 CaBr_2 | 3 | 3 The rate term for each chemical species, B_i, is 1/ν_i(Δ[B_i])/(Δt) where [B_i] is the amount concentration and t is time: chemical species | c_i | ν_i | rate term CaSO_4 | 3 | -3 | -1/3 (Δ[CaSO4])/(Δt) AlBr_3 | 2 | -2 | -1/2 (Δ[AlBr3])/(Δt) Al_2(SO_4)_3 | 1 | 1 | (Δ[Al2(SO4)3])/(Δt) CaBr_2 | 3 | 3 | 1/3 (Δ[CaBr2])/(Δt) (for infinitesimal rate of change, replace Δ with d) Set the rate terms equal to each other to arrive at the rate expression: Answer: | | rate = -1/3 (Δ[CaSO4])/(Δt) = -1/2 (Δ[AlBr3])/(Δt) = (Δ[Al2(SO4)3])/(Δt) = 1/3 (Δ[CaBr2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: CaSO_4 + AlBr_3 ⟶ Al_2(SO_4)_3 + CaBr_2 Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the rate term for each chemical species. • Write the rate of reaction expression. Write the balanced chemical equation: 3 CaSO_4 + 2 AlBr_3 ⟶ Al_2(SO_4)_3 + 3 CaBr_2 Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i CaSO_4 | 3 | -3 AlBr_3 | 2 | -2 Al_2(SO_4)_3 | 1 | 1 CaBr_2 | 3 | 3 The rate term for each chemical species, B_i, is 1/ν_i(Δ[B_i])/(Δt) where [B_i] is the amount concentration and t is time: chemical species | c_i | ν_i | rate term CaSO_4 | 3 | -3 | -1/3 (Δ[CaSO4])/(Δt) AlBr_3 | 2 | -2 | -1/2 (Δ[AlBr3])/(Δt) Al_2(SO_4)_3 | 1 | 1 | (Δ[Al2(SO4)3])/(Δt) CaBr_2 | 3 | 3 | 1/3 (Δ[CaBr2])/(Δt) (for infinitesimal rate of change, replace Δ with d) Set the rate terms equal to each other to arrive at the rate expression: Answer: | | rate = -1/3 (Δ[CaSO4])/(Δt) = -1/2 (Δ[AlBr3])/(Δt) = (Δ[Al2(SO4)3])/(Δt) = 1/3 (Δ[CaBr2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| calcium sulfate | aluminum tribromide | aluminum sulfate | calcium bromide formula | CaSO_4 | AlBr_3 | Al_2(SO_4)_3 | CaBr_2 Hill formula | CaO_4S | AlBr_3 | Al_2O_12S_3 | Br_2Ca name | calcium sulfate | aluminum tribromide | aluminum sulfate | calcium bromide IUPAC name | calcium sulfate | tribromoalumane | dialuminum trisulfate | calcium dibromide
| calcium sulfate | aluminum tribromide | aluminum sulfate | calcium bromide formula | CaSO_4 | AlBr_3 | Al_2(SO_4)_3 | CaBr_2 Hill formula | CaO_4S | AlBr_3 | Al_2O_12S_3 | Br_2Ca name | calcium sulfate | aluminum tribromide | aluminum sulfate | calcium bromide IUPAC name | calcium sulfate | tribromoalumane | dialuminum trisulfate | calcium dibromide

Substance properties

| calcium sulfate | aluminum tribromide | aluminum sulfate | calcium bromide molar mass | 136.13 g/mol | 266.69 g/mol | 342.1 g/mol | 199.89 g/mol phase | | solid (at STP) | solid (at STP) | solid (at STP) melting point | | 96 °C | 770 °C | 730 °C boiling point | | 265 °C | | 810 °C density | | 3.205 g/cm^3 | 2.71 g/cm^3 | 3.353 g/cm^3 solubility in water | slightly soluble | reacts | soluble | soluble odor | odorless | | |
| calcium sulfate | aluminum tribromide | aluminum sulfate | calcium bromide molar mass | 136.13 g/mol | 266.69 g/mol | 342.1 g/mol | 199.89 g/mol phase | | solid (at STP) | solid (at STP) | solid (at STP) melting point | | 96 °C | 770 °C | 730 °C boiling point | | 265 °C | | 810 °C density | | 3.205 g/cm^3 | 2.71 g/cm^3 | 3.353 g/cm^3 solubility in water | slightly soluble | reacts | soluble | soluble odor | odorless | | |

Units

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